Question:
How many Faradays are required for the oxidation of one mole of \( \text{H}_2\text{O} \) to \( \text{O}_2 \)?
How many Faradays are required for the oxidation of one mole of \( \text{H}_2\text{O} \) to \( \text{O}_2 \)?
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The number of Faradays required for a reaction is determined by the number of electrons transferred during the reaction. One mole of electrons corresponds to one Faraday.
Updated On: Feb 17, 2025
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Solution and Explanation
The oxidation of \( \text{H}_2\text{O} \) to \( \text{O}_2 \) involves the following reaction:
\[
2 \text{H}_2\text{O} \rightarrow \text{O}_2 + 4 \text{H}^+ + 4e^-
\]
Since 4 electrons are involved in the oxidation of 2 moles of water, the number of Faradays required for 1 mole of \( \text{H}_2\text{O} \) to produce 1 mole of \( \text{O}_2 \) is 4.
Thus, 4 Faradays are required.
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